Welcome to AP Chemistry! I am looking forward to working with you next year. In order for you to be prepared to take on the challenges of AP Chemistry, I have prepared the following assignment for you to complete during the next two months. If you should have any difficulty with any portion of the assignment, please feel free to contact me via email at lisa.cole@bufordcityschools.org
Please complete the exercises and problems contained in the “AP Chemistry Summer Assignments and
Review Material” in preparation for next year. The material is general information that you should know from 1 st year chemistry. In case you have forgotten some of it, I have included general notes and resource materials that should assist you. The material will be reviewed briefly at the beginning of the course in the fall, but the stronger your foundation and the more knowledge you bring to the course, the easier you will find the new material.
The work that you complete in the packet will be collected the first day of class in August and will be graded.
Good luck and I look forward to working with you next year.
Ms. Cole

Summer Assignments and Review Material
Notes: Metric Prefixes and Conversions tera- (T-) 10
12
1 trillion giga- (G-) 10 9 1 billion mega- (M-) 10
6
1 million kilo- (k-) 10
3
1 thousand hecto- (h-) 10
2
1 hundred deka- (da-)** 10 1 ten deci- (d-) 10 -1 1 tenth centi- (c-) 10
-2
1 hundredth milli- (m-) 10
-3
1 thousandth micro- (µ-) 10
-6
1 millionth nano- (n-) 10
-9
1 billionth pico- (p-) 10 -12 1 trillionth femto- (f-) 10
-15
1 quadrillionth
Problems:
1. Perform each of the following conversions.
A. 8.43 cm to meters.
B. 2.41 x 10 2 cm to meters.
C. 294.5 nm to centimeters.
D. 1.445 x 10 4 m to kilometers.
E. 235.3 m to millimeters.
F. 903.3 nm to micrometers.
G. 6.50 x 10 2 terameters to nanometers
H. 1 microgram to picograms
I. 25 femtograms to kilograms
J. 8.0 dm 3 to liters

2. A mole of helium gas contains 6.02 x 10 23 helium atoms. How many helium atoms are there in a millimole of helium? In a kilomole?
Notes: Significant Digits
Rules for Counting Significant Digits:
1.
Nonzero integers are always significant.
2.
Zeroes between significant digits are significant.
3.
Leading zeroes (zeroes that precede all nonzero digits) are never significant.
4.
Trailing zeroes (zeroes at the right end of the number) are significant only if the number contains a decimal point.
5.
Exact numbers (numbers obtained by counting instead of measuring) have an infinite number of significant digits.
Rules for Significant Digits in Mathematical Operations:
1.
Multiplication and Division: The number of significant digits in the answer is the same as the number of significant digits in the least precise measurement used in the calculation.
2.
Addition and Subtraction: The number of significant digits in the answer has the same number of decimal places as the least precise measurement used in the calculation.
Problems:
1. How many significant digits are in each of the following? a. 12 b. 2001 c. 2.001 x 10 3 d. 0.0400101 e. 0.0048 f. 0.00480 g. 100 h. 100.00

2. Use exponential notation to express the number 480 to a. one significant digit b. two significant digits c. three significant digits d. four significant digits
3. Perform the following mathematical operations and express each result to the correct number of significant digits. a. 4.184 x 100.62 x (25.57-24.16) b. (9.04 – 8.23 + 21.954 + 81.0) / 3.1416 c. 0.1654 + 2.07 + 2.114 d. (9.5 + 4.1 + 2.8 + 3.175) / 4 e. 0.102 x 0.0821 x 273 / 1.01 f. 0.14 x 6.022 x 10 23
Notes: Density and Temperature Conversion
Density = mass/ volume
1 cm 3 = 1 mL and 1 dm 3 = 1 L
Kelvin = o C + 273
Problems:
1. A rectangle has dimensions 2.9 cm x 3.5 cm x 10.0 cm. The mass of the block is
615.0 g. What are the volume and density of the block?
2. A sample containing 33.42 g of metal pellets is poured into a graduated cylinder containing 12.7 mL of water, causing the water level in the cylinder to rise to 21.6 mL. Calculate the density of the metal.
3. Convert the following Celsius temperatures to Kelvin. a. the boiling point of ethyl alcohol, 78.1
b. a cold wintery day, -25 o C o C c. the lowest possible temperature. -273 o C d. the melting point of sodium chloride, 801 o C

Notes: Periodic Table
Horizontal rows on the table are called periods. Vertical columns are called groups.
The groups are identified by number and by name. The groups are numbered from left to right. The names for the groups are:
Group 1: Alkali Metals
Group 2: Alkaline Earth Metals
Group 16: Chalcogens
Group 17: Halogens
Group 18: Noble Gases
Groups 3-12: Transition Elements
The metals are found on the left and in the middle of the table, and the nonmetals are found on the right side of the table.
Problems:
1. List the noble gas elements. Which of the noble gases has only radioactive isotopes? (This is indicated on most periodic tables by parentheses around the mass of the element.)
2. In the periodic table, how many elements are found in a. the second period? b. the third period? c. the fourth period? d. Group 5A?
3. What are the symbols for the following elements: a. gold h. sodium b. silver i. calcium c. mercury d. potassium e. iron f. antimony g. tungsten j. chlorine k. nickel l. strontium m. chromium n. aluminum

Notes: Atomic Structure
Atoms are made up of three subatomic particles. The proton is positively charged and is located in the nucleus of the atom. The neutron has no charge and is also located in the nucleus. The electron is negatively charged and orbits the nucleus in the empty space surrounding the nucleus of the atom. The atomic number is the number of protons. Since atoms are electrically neutral, the number of protons is equal to the number of electrons. The mass number is the number of particles in the nucleus (the number of protons and neutrons). Isotopes are atoms of the same element having different atomic masses due to differing numbers of neutrons.
Isotope symbols, such as the one shown below, are often used to determine the structure of an atom.
23
11
Na
11 protons
11 electrons
12 neutrons
A- mass number = # of protons + # of neutrons
Z- atomic number = # of protons (found on periodic table)
Cations are formed when atoms lose electrons resulting in the atom having a positive charge. Anions are formed when atoms gain electrons which results in a negative charge.
Problems:
1.
Complete the following table:
Symbol Number of Number of
238
92
U
89
39
Y protons
20
23 neutrons
20
28
35 44
15 16
Number of electrons
20
36
Net Charge
2+
3-

2. Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion is the most likely in each case? a. Ra d. Te b. In e. Br c. P f. Rb
Notes: Naming Compounds/Formula Writing
When naming binary ionic compounds (those containing a metal and a nonmetal), the metal is named first followed by a name derived from the root name of the nonmetal (the ending is usually changed to –ide). If the metal can form more than one cation (usually a transition element), the metal name is followed by a Roman numeral that indicates the cation charge. Polyatomic ions have special names that must be memorized along with their charges. (A list of polyatomic ions is attached at the end of this packet.) In compounds containing polyatomic ions, the cation name is given first followed by the anion name. For binary covalent compounds
(those containing two nonmetals), the first element is named using the entire element name and the second element is named as if it were an anion. Prefixes are used to indicate the numbers of atoms present.
Prefixes Used to Indicate Subscripts in Covalent Molecules
6
7
8
9
10
3
4
5
Prefix
1
2
Number
Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca

Problems:
1. Name each of the following compounds: a. NaCl h. CaS b. Rb
2 c. CsF d. Ag
2 e. TiO
O
S
2 i. AlI j. Li
3
3
N k. MnO
2 l. Sr
3
P
2 f. NI
3 g. SF
2
2. Name each of the following compounds: a. HC
2 b. NH
4 c. CO
2 f. KIO
H
S
3
3
O
2
NO
2
3 d. ICl e. Pb
3
(PO
4
)
2 m. PCl
3 n. N
2
F
4 g. H
2
SO
4 h. Sr i. Al
2
3
(SO
3 j. SnO k. Na
2
N
2 l. HClO
2
)
CrO
4
3
3. Write the formula for each of the following compounds: a. cesium bromide e. silicon tetrachloride b. barium sulfate c. ammonium chloride f. chlorine trifluoride g. beryllium oxide d. chlorine monoxide h. magnesium fluoride
4. Write the formula for the following compounds: a. ammonium hydrogen phosphate b. mercury (I) sulfide c. silicon dioxide d. sodium sulfite e. aluminum hydrogen sulfate f. nitrogen trichloride g. hydrobromic acid h. bromous acid i. perbromic acid j. potassium hydrogen sulfide k. calcium iodide l. cesium perchlorate

Notes: Mole Concept
A mole is a unit of measure equal to the number of carbon atoms in exactly 12 grams of pure carbon-12. This number has been determined experimentally to be
6.02214 x 10 23 , which is called Avogadro’s number. One mole of any substance contains Avogadro’s number of units. One mole of an element has a mass equal to the element’s atomic mass in grams.
Problems:
1. Calculate the molar mass of the following substances. a. NH
3 b. N
2
H c. (NH
4
4
)
2
Cr
2
O
7
2. How many moles of compound are present in 1.00 g of each of the compounds in the problem above?
3. How many molecules (or formula units) are present in 1.00 g of each of the compounds in problem 1?
Notes: Balancing Equations
Atoms are conserved in chemical reactions. The same number of each type of atom must be found among the reactants and products. In order for equations to adequately represent the reactions that are actually taking place, they must often be balanced. The formulas of the compounds must never be changed in balancing a chemical equation. That is, the subscripts in a formula cannot be changed. Only coefficients can be added.

Balancing Equations
Balance the following equations. Use the smallest possible coefficients. Identify the type of reaction.
1. K + Cl
2
 KCl

NaNO
2
+ O
2
2. NaNO
3
O
2

H
2
O 3. H
2
+
4. Br
2
+ KI  KBr + I
2
5. Al +
6. C
3
H
8
+
7. AgNO
3
HCl
O
+
2


MgCl
2
AlCl
CO
2
3
+
+

H
H
2
2
O
AgCl + Mg(NO
3
)
2
8. H
2
O
2
 H
2
O +
9. AlBr
3
+ K
2
SO
4
O
2
10. C
4
H
10
11. P
4
O
10
12. Na
3
PO
4
+
+
+
O
H
2
2
O
BaCl
2



CO
H

3
2
PO
4
KBr
+
Ba
3
+
H
(PO
4
2
)
O
2
Al
+
2
(SO
4
)
3
NaCl

Notes: Problem Solving and Logical Thinking
Problem solving skills will be necessary in order to be successful in this class. In order to begin developing your logical thinking skills, try to solve the logic problems that are included in this packet.
Logic Problem #1
Lab Assistants
Dr Beaker is supervising four students. All the students, named Beryl, Selena, Al and Mo, will produce a compound of a different color; black, white, red or green.
One student is working in the organic lab, one in the inorganic lab, one in the physical lab and one in the analytical lab. The building has four floors labeled 1, 2,
3 and 4, and each lab is situated on a different floor.
1. Mo works on an odd numbered floor.
2. The student who made the white compound works in the physical lab.
3. Al works one floor above Mo.
4. The black compound was made on the floor above the white one by Selena, who is an analytical chemist.
5. Beryl works on the floor which is immediately above the organic chemist and immediate below the analytical chemist.
6. The organic chemist has to use the stairs to get to their lab.
7. Al made the green compound and is meeting the inorganic chemist after work.
Can you help Dr Beaker decide which student is in which lab, on which floor and what the color of their compound should be?

Logic Problem #2
Magic Circle
By Nobuyuki Yoshigahara
Eight numbers are placed in the diagram shown below. Do you see a pattern in going from one number to the next as you follow the arrows? Describe the pattern and identify the missing number.
37
58
16
4 89
145
?
42

Logic Problem #3
4 quarts 2 ½ quarts 1 ½ quarts
A milk pitcher contains 4 quarts of milk. The milk needs to be divided equally between two friends. The only containers available are two empty bottles, one of them which holds 2 ½ quarts and the other which holds 1 ½ quarts. Using the pitcher and both bottles, explain how the milk can be divided equally between the two friends.

Are you ready for the challenge of AP Chemistry?
The following problems are based on the concepts covered in Honors Chemistry; however, the difficulty level is representative of what you will see in AP Chemistry.
Try to solve them and see if you are ready for the challenge. Good Luck!
1. If you put 8.21 gallons of gas in your car and it cost you a total of $17.25, what
is the cost of gas per liter in Canadian dollars? Assume 0.82 dollar U.S. = 1.00
dollar Canadian. (Solve using the Factor Label Method)
2. Using the information given below, answer the following questions. In an ion
with an unknown charge, the total mass of all electrons was determined to be
2.55 x 10 -26 g , while the total mass of its protons was 5.34 x 10 -23 g. What is
the identity and charge on this ion? What is the symbol and mass number of a
neutral atom whose total mass of its electrons is 3.92 x 10 -26 g, while its
neutrons have a mass of 9.35 x 10 -23 g? mass of electron = 9.11 x 10 -31 kg mass of proton = 1.67 x 10 -27 mass of neutron = 1.67 x 10 kg
-27 kg
3. A binary compound is known to contain a cation with 51 protons and 48 electrons.
The anion contains one-third the number of protons as the cation. The number
of electrons in the anion is equal to the number of protons plus 1. What is the
formula of this compound? What is the name of this compound?
4. A given sample of a xenon fluoride compound contains molecules of the type
XeF n
, where n is some whole number. Given that 9.03 x 10 20 molecules of
XeF n
weighs 0.368 g, determine the value of n in the formula and identify the
geometric shape of the molecule.
5. An ionic compound MX
3
is prepared according to the following unbalanced
chemical equation.
A 0.105 g sample of X
2
M + X
2
 MX
3
contains 8.92 x 10 20 molecules. The compound MX
3
consists of 54.47% X by mass. What are the identities of M and X, and what is
the correct name for MX
3
? Starting with 1.00 g each of M and X
2
, what mass
of MX
3
can be prepared?

6. A 20.0 L stainless steel container was charged with 2.00 atm of hydrogen gas
and 3.00 atm of oxygen gas. A spark ignited the mixture, producing water.
What is the pressure in the tank at 25 o C? at 125 o C?
7. Tris(pentafluorophenyl)borane, commonly known by its acronym BARF, is
frequently used to initiate polymerization of ethylene or propylene in the
presence of a catalytic transition metal compound. It is composed solely of
C, F, and B; it is 42.23% C by mass and 55.66% F by mass.
a) What is the empirical formula of BARF?
b) A 2.251 g sample of BARF dissolved in 347.0 mL of solution produces a
0.01267 M solution. What is the molecular formula of BARF?
8. An unknown compound contains only C, H, and O. Combustion analysis of the
compound gives mass percentages of 31.57% C and 5.30% H. The molar mass
is determined by freezing point depression of an aqueous solution. A freezing
point of -5.20
o C is recorded for a solution made by dissolving 10.56 g of the
compound in 25.0 g water. Determine its empirical formula, molar mass, and
molecular formula of the compound. Assume that the compound is a non-
electrolyte. (K f
of water is 1.86 o C .
kg/mol)
***If you could not solve these problems, please do not let it discourage you from taking the course. You each have come highly recommended and are capable of doing well and achieving much success in the class. I simply wanted to give you a sneak preview of the problem-solving that will be taking place in the class on a daily basis. I am excited about your willingness to take on this challenge and am looking forward to a great year!

Anions
1-
Acetate, CH
3
COO -
Amide, NH
2
-
Azide, N
3
-
Benzoate, C
6
H
5
COO -
Chlorate, ClO
3
-
Chlorite, ClO
2
-
Cyanate, OCN -
Cyanide, CN -
Dihydrogen phosphate,
H
2
PO
4
-
Formate, HCOO -
Hydrogen carbonate
(bicarbonate), HCO
3
-
Hydrogen sulfate
(bisulfate), HSO
4
-
Hydrogen sulfide
(bisulfide), HS -
Hydroxide, OH -
Hypochlorite, ClO -
Iodate, IO
3
-
Nitrate, NO
3
-
Nitrite, NO
2
-
Perchlorate, ClO
4
-
Permanganate, MnO
4
-
Thiocyanate, SCN -
Triiodide, I
3
-
Vanadate, VO
3
-
Common Polyatomic Ions
2-
Carbide, C
2
2-
Carbonate, CO
3
2-
Chromate, CrO
4
2-
Dichromate, Cr
2
O
7
2-
Imide, NH 2-
Manganate, MnO
4
2-
Metasilicate, SiO
3
2-
Monohydrogen phosphate,
HPO
4
2-
Oxalate, C
2
O
4
2-
3-
Aluminate, AlO
3
3-
Arsenate. AsO
4
3-
Borate, BO
3
3-
Citrate, C
6
H
5
O
7
3-
Phosphate, PO
4
3-
Phosphite, PO
3
3-
Peroxide, O
2
2-
Peroxydisulfate, S
2
O
8
2-
4-
Orthosiliscate, SiO
4
4-
Phthalate, C
8
H
4
O
4
2-
Polysulfide, S x
2-
Selenate, SeO
4
2-
Sulfate, SO
4
2-
Sulfite, SO
3
2-
Tartrate, C
4
H
4
O
6
2-
Tellurate, TeO
4
2-
Tetraborate, B
4
O
7
2-
Thiosulfate, S
2
O
3
2-
Tungstate, WO
4
2-
Zinvate, ZnO
2
2-
Pyrophosphate, P
5-
Tripolyphosphate, P
3
O
10
5-
Cations
1+
Ammonium, NH
4
+
Hydronium, H
3
O +
2
O
7
4-